Textbook Question
From a plot of the concentration–time data in Worked Example 14.9, estimate: (b) the initial rate of decomposition of NO2.
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Ch.14 - Chemical Kinetics
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 14, Problem 58
Chlorite is reduced by bromide in acidic solution according to the following balanced equation: ClO2 -1aq2 + 4 Br-1aq2 + 4 H+1aq2S Cl-1aq2 + 2 Br21aq2 + 2 H2O1l2(a) If Δ3Br24>Δt = 4.8 * 10-6 M>s, what is the value of Δ3ClO2 -4>Δt during the same time interval?
Verified step by step guidance1
Identify the stoichiometry of the reactants in the balanced chemical equation. For every 1 mole of ClO2-, 4 moles of Br- are required.
Determine the rate of consumption of Br- from the given rate of formation of Br2. Since 2 moles of Br- produce 1 mole of Br2, the rate of consumption of Br- is twice the rate of formation of Br2.
Apply the stoichiometric relationship between ClO2- and Br- to find the rate of consumption of ClO2-. Since 4 moles of Br- correspond to 1 mole of ClO2-, divide the rate of consumption of Br- by 4 to find the rate of consumption of ClO2-.
Express the rate of consumption of ClO2- with the correct sign, as it is being consumed in the reaction. The rate should be negative, indicating a decrease in concentration over time.
Ensure the units of the rate of consumption of ClO2- are consistent with the units given for the rate of formation of Br2, which is M/s (molarity per second).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to determine how much of each substance is consumed or produced based on the balanced chemical equation. In this case, understanding the stoichiometric coefficients of ClO2 and Br- in the reaction is essential to relate their rates of change.
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Stoichiometry Concept
Rate of Reaction
The rate of reaction refers to the speed at which reactants are converted into products in a chemical reaction. It is typically expressed as the change in concentration of a reactant or product over time. In this question, the rate of change of bromide (Δ[Br-]/Δt) is given, and we need to use stoichiometry to find the corresponding rate of change for chlorite (Δ[ClO2-]/Δt).
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Concentration and Molarity
Concentration is a measure of the amount of a substance in a given volume of solution, commonly expressed in molarity (M), which is moles of solute per liter of solution. Understanding how to manipulate and convert concentrations is crucial for calculating the rates of change in this reaction. The given rate for bromide will help us determine the rate for chlorite by applying the stoichiometric ratios from the balanced equation.
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Related Practice
Textbook Question
Ammonia is manufactured in large amounts by the reaction N21g2 + 3 H21g2S 2 NH31g2 (b) How is the rate of formation of NH3 related to the rate of consumption of N2?
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Textbook Question
Ammonia is manufactured in large amounts by the reaction
N2(g) + 3 H2(g) → 2 NH3(g)
(a) How is the rate of consumption of H2 related to the rate of consumption of N2?
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Textbook Question
The reaction 2NO1g2 + 2 H21g2S N21g2 + 2 H2O1g2 is first order in H2 and second order in NO. Write the rate law, and specify the units of the rate constant.
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Textbook Question
Initial rate data at 25 °C are listed in the table for the reaction NH4 +1aq2 + NO2 -1aq2S N21g2 + 2 H2O1l2 (b) What is the value of the rate constant?
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Textbook Question
Trimethylamine and chlorine dioxide react in water in an electron transfer reaction to form the trimethylamine cation and chlorite ion: 1CH323 N1aq2 + ClO21aq2 + H2O1l2S 1CH323 NH+1aq2 + ClO2 -1aq2 + OH-1aq2 Initial rate data obtained at 23 °C are listed in the following table. (b) What would be the initial rate in an experiment with initial concentrations 31CH323 N4 = 4.2 * 10-2 M and 3ClO24 = 3.4 * 10-2 M?